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3 years ago

Which determines the reactivity of an alkali metal?

Chemistry

2 answers:

marissa [1.9K]3 years ago

8 0

Answer: D— the ability to lose electrons

Explanation:

Just took the quiz

adelina 88 [10]3 years ago

3 0

Answer:

its ability to lose electron

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Which is the least viscous? A C20H42 B. CCL4 C. CH3OH D. CHCI3 E. C6H6

velikii [3]

C. CH3OH
hope this helped! :))

7 0

3 years ago

Magnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to form magnesium chloride and iron. 3Mg(s) +

Paladinen [302]

Answer:

Theanswer to your question is:

Limiting reactant = FeCl₃

Excess reactant = 1.66 g of Mg

Explanation:

Data

Mg = 41 g = 24.31 g/mol

FeCl₃ = 175 g = 162.2 g/mol

3Mg(s) + 2FeCl₃(s) → 3MgCl₂(s) + 2Fe(s)

3(24.31) of Mg ------------------ 2(162.2) of FeCl₃

72.93 g of Mg ------------------ 324.4 g of FeCl₃

Theoretical Proportion = 324.4/72.93 = 4.44

Practical proportion = 175 / 41 = 4.2

As the proportion disminishes the limiting reactant is FeCl₃.

Excess reactant

72.93 g of Mg ------------------ 324.4 g of FeCl₃

x ------------------------- 175 g of FeCl₃

x = (175 x 72.93) / 324.4

x = 39.34 g of Mg

Excess = 41 - 39.34

= 1.66 g of Mg

4 0

3 years ago

Which best describes the relationships between subatomic particles in any neutral atom? * 1 point the number of electrons equals

Anna71 [15]

Atomic number = protons

Protons = P Electrons = E P = E

Atomic mass = Neutrons + Protons

Atomic number = atomic mass = neutrons

P = E

AM - AN = N

Example:

Calcium = 20 Protons 20P = 20E

Atomic mass - atomic number = neutrons :)

4 0

4 years ago

Zn + 2 HCl → ZnCl2 + H2

MrRissso [65]

Answer:

10.1g of H₂ are produced

Explanation:

To solve this question we need, first, to convert the mass of each reactant to moles and, using the chemical reaction, find limiting reactant. With limiting reactant we can find the moles of H2 and its mass:

Moles Zn -Molar mass: 65.38g/mol-:

307g * (1mol / 65.38g) = 4.696 moles

Moles HCl -Molar mass: 36.46g/mol-:

381g HCl * (1mol / 36.46g) = 10.45 moles

For a complete reaction of 10.45 moles of HCl are required:

10.45 moles HCl * (1mol Zn / 2mol HCl) = 5.22 moles Zn

As there are 4.696 moles of Zn, Zn is the limiting reactant

The moles of H₂ produced = Moles of Zn added = 4.696 moles. The mass is-Molar mass H₂ = 2.16g/mol-:

4.696 moles * (2.16g / mol) =

<h3>10.1g of H₂ are produced</h3>

7 0

3 years ago

Please help with chemistry question... It would help me tremendously and if you can, please show work :)?

Alexxandr [17]

Answer:

5.06 atm

Explanation:

Step 1:

Data obtained from the question. This includes:

Mass of S2O = 175g

Volume (V) = 16600 mL

Temperature (T) = 195°C

Pressure (P)

Step 2:

Determination of the number of mole of S2O in 175g of S2O.

Mass of S2O = 175g

Molar Mass of S2O = (32x2) + 16 = 64 + 16 = 80g/mol

Number of mole of S2O =.?

Number of mole = Mass/Molar Mass

Number of mole of S2O = 175/80

Number of mole of S2O = 2.1875 moles

Step 3:

Conversion to appropriate units.

It is essential to always express the various variables in the right units of measurement in order to obtain the desired answer in the right units.

For volume:

1000mL = 1L

Therefore, 16600mL = 16600/1000 = 16.6L

For temperature:

Temperature (Kelvin) = temperature (celsius) + 273

Temperature (celsius) = 195°C

Temperature (Kelvin) = 195°C + 273 = 468K

Step 4:

Determination of the pressure.

The pressure can be obtained by the application of the ideal gas equation. This is illustrated below:

Volume (V) = 16.6L

Temperature (T) = 468K

Number of mole (n) = 2.1875 moles

Gas constant (R) = 0.082atm.L/Kmol

Pressure (P) =

PV = nRT

P x 16.6 = 2.1875 x 0.082 x 468

Divide both side by 16.6

P = (2.1875 x 0.082 x 468) /16.6

P = 5.06 atm

Therefore, the pressure is 5.06 atm

6 0

4 years ago